Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to th

Question

Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following equation: 2NO + 2H_2 rightarrow N_2 + 2H_2O The experimental rate law is Rate = k[NO]^2[H_2]. If time is measured in minutes and concentration is measured in moles per liter, what are the units for the rate of consumption of hydrogen? A) mol/(L middot min). B) mol/(L^2 middot min). C) L^2/(mol^2 middot min). D) mol^2/(L^2 middot min). E) mol^3/(L^3 middot min). Which of the following corresponds to the correct integrated expression for a first-order reaction? A) 1/A - 1/B = kt B) 1/A - 1/A_0 = kt C) 1/A_0 - ln A/A_0 = kt D) ln A - ln A_0 = -kt E) t_1/2 = 0.693/k The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH_3(g) + 3O_2(g) rightarrow 2N_2(g) + 6H_2O(I) Suppose the rate of formation of H_2O(I) is 3.0 mol/(L middot s). Which of the following statements is true? A) The rate of formation of N_2 is 2.0 mol/(L middot s). B) The rate of consumption of NH_3 is 2.0 mol/(L middot s). C) The rate of consumption of O_2 is 2.0 mol/(L middot s). D) The rate of consumption of NH_3 is 0.50 mol/(L middot s). E) The rate of formation of N_2 is 1.3 mol/(L middot s).

Explanation / Answer

1. This is third order reaction. So, Concentration to the power 3 and divide by single power of time. So option e.

2. First order reaction

Rate=d[A]/dt=k[A]
Integrate the above equation from Ao To A

ln[A]-ln[A]o=kt

So, equation d is correct

3. Rate of formation of H20= Rate of consuming NH3
1/6(d H2O/dt) = -1/4 (d NH3/dt)
1/6*3= -1/4*x
x=2

So, option b

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